the above reaction can b divided into
i) Zn(s) - 2e- ---> Zn2+(aq) [E degree reduction = - .76V]
ii) Ni2+(aq) + 2e- ---> Ni(s) [E degree reduction > - .76V]
from the reactions v can say that Zn is more reactive than Ni. This is because Zn is oxidised in preference to Ni as reduction potential of Zn2+ is more negative than that of Ni2+. Since in a redox reaction , both oxidation & reduction occur , so Ni2+ is reduced as oxidation has already occured .

Zn+Ni^2= Zn (subscript 2)Ni....but there are some expections...some books include Zinc as a transition element...so, if its a transition element, the its written this way: ZN(II)Ni....THE (II) is in roman numeral form

all the peeps who are saying something about 'more reactive' haven't taken chem in a while (neither is 'more' reactive than the other)

one is oxidized, one is reduced, (nickel and zinc, respectively), one is an oxidizing agent, the other is a reducing agent (the reverse, respectively)

that if this reaction is happening at standard conditions, it would be spontaneous, as E is positive

that if this was set up in a lab as an electrochemical cell with all associated parts (salt bridge, etc), that the zinc would be going into solution while the Nickel would be accumulating in solid form - and by one convention, the zinc would be the anode (because that is where oxidation occurs) and the nickel the cathode, but by the convention of 'electron flow' those lables would be reversed

Source(s):

zn is acting as a reducing agent and nickel as an oxidizing agent.
Zn gives out two ectrons to nickel and get oxidized. Ni accepts two electrons and get reduced. In a redox reaction, oxidizing agent get reduzed and reducing agent get oxidized.

Source(s):

the above reaction can b divided into
i) Zn(s) - 2e- ---> Zn2+(aq) [E degree reduction = - .76V]
ii) Ni2+(aq) + 2e- ---> Ni(s) [E degree reduction > - .76V]
from the reactions v can say that Zn is more reactive than Ni. This is because Zn is oxidised in preference to Ni as reduction potential of Zn2+ is more negative than that of Ni2+. Since in a redox reaction , both oxidation & reduction occur , so Ni2+ is reduced as oxidation has already occured .

zinc is oxidized n nikel is reduced..u can actually notice that the oxidation number of zinc increase from 0 to +2 and the oxidation number for nikel decreases from +2 to 0.
hence, nikel is the oxidizing agent because it release 2 electrons to oxidize zinc while zinc is the reducing agent because it accepts 2 electrons frm nikel to reduce nikel